Question

Ph of a 5 into 10 to the power minus 6 moles of barium hydroxide solution is

Answer 1

9is ur answer ,,,,,,,,

Answer 2

pH of a $5\times10^{-6}$ moles of $Ba(OH)_2$ solution is 9

Given:

Concentration of solution = $5\times10^{-6}$ Moles

To find:

pH = ?

Formula to be used:

pOH = -$log[OH]^-$

pH = 14-pOH

Calculation:

When $Ba(OH)_2$, it leads to the formation of given products

$Ba(OH)_2\rightarrow Ba^{2+}+2OH^-$

As $Ba(OH)_2$ is a base, the $OH^-$ concentration must be taken into account and to calculate pH, first pOH value must be calculated.

Accordingly,

$Ba(OH)_2$ = $5\times10^{-6}$

$2OH^-$ = 2×( $5\times10^{-6}$) = $1\times 10^{-5}$

Substituting the obtained value in the pOH formula, it gives pOH values which is as follows:

pOH = -$log[OH]^-$

pOH = $-log ({1\times10^{-2})$

pOH = 5

∵ pOH = 5

∴ pH = 14 - pOH

pH = 14-5

pH = 9

Conclusion:

Thus pH of  $5\times10^{-6}$ moles of $Ba(OH)_2$ solution is calculated as 9.

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